Compare krypton and bromine in terms of chemical stability.

To compare krypton and bromine in terms of chemical stability, we need to consider their positions in the periodic table, their electron configurations, and their reactivity. 1. **Position in the Periodic Table:** - Krypton (Kr) is a noble gas located in Group 18 (or Group 0) of the periodic table. - Bromine (Br) is a halogen located in Group 17. 2. **Electron Configuration:** - Krypton has the electron configuration of \([Ar] 3d^{10} 4s^2 4p^6\), which means it has a full outer shell of electrons (8 electrons in the outermost shell). - Bromine has the electron configuration of \([Ar] 3d^{10} 4s^2 4p^5\), which means it has 7 electrons in its outer shell and is one electron short of achieving a full outer shell. 3. **Chemical Stability:** - **Krypton:** Due to its full outer electron shell, krypton is chemically stable and generally unreactive. Noble gases are known for their lack of reactivity because they do not tend to gain, lose, or share electrons. - **Bromine:** Bromine, on the other hand, is more reactive because it seeks to gain one electron to achieve a stable octet configuration. This makes bromine more likely to participate in chemical reactions, especially with metals and other nonmetals. 4. **Conclusion:** - Krypton is more chemically stable than bromine due to its full outer electron shell, making it largely inert. In contrast, bromine is less stable and more reactive because it is one electron short of a full outer shell. In summary, krypton is chemically stable and unreactive, while bromine is reactive and less stable due to its incomplete outer electron shell.